Year 10 CHEMISTRY (IGCSE) LONG TERM PLAN with CURRICULUM STANDARDS
Year 10
CHEM
WEEK 1
WEEK 2
Y 10/CHE (6)
States of matter
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Year 10
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Year 10
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Year 10
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WEEK 3
WEEK 4
WEEK 5
Y 10/CHE (8)
Y 10/CHE (4)
Elements,compounds and mixtures Atomic structure
Classify a substance as an element, compound or
Baseline Compare the arrangement and
movement
of
particles
in
solid,liquid
mixture.Analyse paper chromatography as the
test
Ellaborate the structure
of an atom in terms of
and gases.Evaluate how the results of separation of mixtures of soluble
the positions, relative
experiments involving the dilution of substances by running a solvent (mobile phase)
masses and
coloured solutions and diffusion of
through the mixture on the paper (the paper
charges of sub-atomic
gases can be explained.Plot and
contains the stationary phase), which causes the
particles.Describe the
interpret solubility curves.Investigate substances to move at different rates over the
structure of an atom in
the solubility of a solid in water at a
paper.Describe the experimental techniques of
terms of the positions,
specific temperature.
separation of mixtures by different techniques like relative masses and
Assessment 1
paper chromatography and distillation.
relative charges of subAssessment 2
atomic particles
WEEK 1
WEEK 6
The periodic table
Deduce the electronic configurations of the first 20 elements from their
positions in the Periodic Table.Identify an element as a metal or a non-metal
according to its position in the Periodic Table.Relate the electronic
configuration of a main group element is related to its position in the
Periodic Table.Reason out why elements in the same group of the Periodic
Table have similar chemical properties.Reason out why the noble gases
(Group 0) do not readily react.Use patterns in the Periodic Table to interpret
data and predict properties of elements.Draw the electron arrangements for
He, Ne and Ar.
Correlate the properties with outer shell electrons.
Assessment 3
WEEK 4
Y 10/CHE (8)
Y 10/CHE (4)
Y 10/CHE (4)
Y 10/CHE (12)
Ionic Bonding
Covalent Bonding
Metallic bonding
Chemical formulae, equations and calculations
Understand how ions are formed by electron loss
or gain.Predict the formulae of ionic compounds
ending with -ide and ate.Draw dot-and-cross
diagrams to show the formation of ionic
compounds by electron transfer, limited to
combinations of elements from Groups 1, 2, 3 and
5, 6, 7 only outer electrons need be shown.Reason
out why compounds with giant ionic lattices have
high melting and boiling points. Assessment 4
Define that a covalent
bond is formed between
atoms by the sharing of a
pair of electrons.Use dotand-cross diagrams to
represent covalent bonds
in simple molecules like
water,carbondioxide.
Know how to represent a
metallic lattice by a 2D
diagram.Predict the
metallic bonding in
terms of electrostatic
attraction.Compare
physical properties
including conductivity
and malleability.
Assessment 5,6
WEEK 3
WEEK 4
WEEK 1
WEEK 2
WEEK 8
Y 10/CHE (12)
WEEK 3
WEEK 2
WEEK 5
WEEK 7
WEEK 6
WEEK 7
WEEK 8
Compare the word and balanced equations for familiar and unfamiliar
REVISION FOR FIRST
reactions.Define one mole of a substance.Identify Avogadro's constant as
TERM EXAM
6.023 × 10 23.Use the formula n=m/Ar or n=m/Mr. Calculate the moles of
particles of a substance.calculate reacting masses using experimental data
and chemical equations.Differentiate between percentage yield and
theoretical yield.Carry out experiments to find the formula of magnesium
oxide.Differentiate between empirical formula and molecular formula.Use
the formula C= n/V to calculate the concentration in g/dm3.Use the formula
n= V/Vm to calculate the amount of gas. Assessment 7
WEEK 5
WEEK 6
WEEK 7
WEEK 8
Y 10/CHE (8)
Y 10/CHE (8)
Y 10/CHE (4)
Y 10/CHE (4)
Y 10/CHE(8)
Group 1 and Group 7
Gases in the atmosphere
Reactivity series
Extraction
Acids,alkalis and titration
Use knowledge of trends in Group 1 to predict the
properties of other alkali metals.Predict the trend
in reactivity in all the members in the group 1 and
7.Write the balanced symbol equation of hydrogen
with halogens with state symbols and predict
reaction of other hydrogen other
halogens.Assessment 8
WEEK 1
WEEK 2
Compare the approximate percentages by volume
of the four most abundant gases in dry air.State
that carbon dioxide and methane are greenhouse
gases and explain how they may contribute to
climate changePlan an investigation to determine
the approximate percentage by volume of oxygen
in air.
WEEK 3
WEEK 4
Describe how metals
can be arranged in a
reactivity series based on
their reactions with
water dilute hydrochloric
or sulfuric acid.
WEEK 5
Outline the method of
separating metals from
their ores.Define an
alloy.Relate the uses of
metals are related to
their properties.
Assessment 9,10
WEEK 6
Y 10/CHE (12)
Y 10/CHE (12)
Acids,bases and salt preparations
Chemical tests
Identify the general rules which describe the solubility in water.Define acids
and bases in terms of proton transfer,in aqueous solutions.Write balanced
chemical equations for the reaction of acids with hydroxides, carbonates and
oxides of the listed metals.Plan an experiment to prepare a pure, dry sample
of a soluble salt, starting from an acid and alkali.Plan an experiment to
prepare a pure, dry sample of an insoluble salt, starting from two soluble
reactants.practical. Prepare a sample of pure, dry hydrated copper(II) sulfate
crystals. Assessment 12
Reasons out why flame test is a ‘qualitative’ method of analysis. Predict why
ions must not give same positive result with two or more different ions.Carry
+
out tests for the cations like NH4 using sodium hydroxide solution and
identifying the gas evolved Cu2+, Fe2+ and Fe3+ using sodium hydroxide
solution.Carry out tests Cl–, Br– and I– using acidified silver nitrate solution
2–
2–
SO4 using acidified barium chloride solution CO3 using hydrochchloric
acid. Assessment 13
Carry out the identification of different types of
acids and alkalis using different types of
indicators.Establish the relationship between
hydrogen ion concentration in a solution and the
pH of the solution.Experiment the titration of
hydrochloric acid with sodium hydroxide.
Asessment 11
WEEK 7
WEEK 8
REVISION FOR FINAL EXAM